Copper(II) sulfate crystals, $\text{CuSO}_4\cdot5\text{H}_2\text{O}$, are hydrated.
Copper(II) sulfate crystals are produced when copper(II) carbonate reacts with dilute sulfuric acid.
The overall equation is given below.
$\text{CuCO}_3 + \text{H}_2\text{SO}_4 + 4\text{H}_2\text{O} \rightarrow \text{CuSO}_4\cdot5\text{H}_2\text{O} + \text{CO}_2$
step 1 Powdered solid copper(II) carbonate is put into 50.0 cm$^3$ of 0.05 mol/dm$^3$ sulfuric acid until copper(II) carbonate is left in excess.
step 2 The surplus copper(II) carbonate is removed from the aqueous copper(II) sulfate.
step 3 The aqueous copper(II) sulfate is heated until the solution becomes saturated.
step 4 The solution is left to cool so that crystals form.
step 5 The crystals are taken out and dried.
(a)[3]
Calculate the greatest mass of the copper(II) sulfate crystals, $\text{CuSO}_4\cdot5\text{H}_2\text{O}$, that can be formed by following these steps.
(b)[1]
Explain why this happened.
(c)[2]
State two observations that would show copper(II) carbonate is in excess in step 1.
(d)[2]
Give a reason for this. Explain your answer using particles.
(e)[1]
Name a different substance, other than copper(II) carbonate, that could be mixed with dilute sulfuric acid in step 1 to make copper(II) sulfate.
(f)[1]
Name the process used when separating the aqueous copper(II) sulfate from excess copper(II) carbonate in step 2.
(g(i))[2]
Suggest what the term saturated solution means.
(g(ii))[1]
What observation would show that the solution was saturated in step 3?
(g(iii))[1]
Why should the aqueous copper(II) sulfate not be heated to dryness in step 3?